Chapter 13, Problem 126IP

Given K = 3.50 at 45°C for the reaction

$\text{A}\left(g\right)+\text{B}\left(g\right)\rightleftharpoons \text{C}\left(g\right)$

and K = 7.10 at 45°C for the reaction

$2\text{A}\left(g\right)+\text{D}\left(g\right)\rightleftharpoons \text{C}\left(g\right)$

what is the value of K at the same temperature for the reaction

$\text{C}\left(g\right)+\text{D}\left(g\right)\rightleftharpoons 2\text{B}\left(g\right)$

What is the value of K_p, at 45°c for the reaction? Starting with 1.50 atm partial pressures of both C and D, what is the mole fraction of B once equilibrium is reached?